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26 Cards in this Set
- Front
- Back
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Weak Electrolyte
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partial ionization or partial dissociation
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BrØnstead-Lowry Acid
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a proton donor
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What is the conjugate acid of a BrØnstead-Lowry Base?
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the conjugate acid is formed when a base accepts a proton
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What is neutralization in terms of BrØnstead-Lowry concept?
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acid/base reaction
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Amphiprotic Solvent
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Species that can either donate or accept a proton
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Autoprotolysis
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the spontaneous reaction of molecules of a substance to give a pair of ions
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Strong Acid
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complete dissociation
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Le Chatelier Principle
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the position of an equilbrium always shifts in such a direction as to relieve a stress that is applied to the system
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Common-Ion Effect
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the reduction in a solublilty of an ionic precipitate when a soluble compound combining one of the ions of the precipitate is added to the solution in equilibrium with the precipitate
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How do you get a conjugate base from an acid?
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remove a H+
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How do you get a conjugate acid from a base?
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add a H+
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How is La Chatelier's principle applied?
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Take out an ion reaction will favor same side.
Add a ion reaction will favor opposite side. |
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What is an electrolyte?
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a solute wich ionizes in a solvent to produce an electrically conducting medium.
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What side of a chemical equations do large K's favor?
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the right side "products"
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What side of a chemical equations do small K's favor?
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the left side "reactants"
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According to the Bronsted-Lowry model how does an acid act in water?
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as a proton donor, it forms H3O+
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According to the Bronsted-Lowry model how does an base act in water?
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as a proton aceptor, the H+ moves from the water to the base
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What do you do if you add chemical equations?
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you multiply the equilbrium constants
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What do you do if you want to switch the aproach on a chemical equation to right to left?
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take the inverse of the equilbrium constant
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When can a charge balance equation be written?
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if the entire chemistry of a system is known
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How can ions in a solution be seperated?
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by using a reagent that will remove one ion from solution by forming a precipitate
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What does solubility of a precipitate do with increases in concentration?
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solubility generally increases
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What happens to Ksp's when varying electrolyte concentration?
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they can vary
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Ionic Strength Equation
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=
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Dilution Equation
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=
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Charge Balance Equation
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=
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